Under which of the following conditions does a gas deviate from ideal behaviour?
$A$. Low pressure
$B$. High pressure
$C$. Low temperature
$D$. High temperature

Explain the physical significance of van der Waals parameters.

At a given temperature $T$,gases $Ne$,$Ar$,$Xe$,and $Kr$ are found to deviate from ideal gas behaviour. Their equation of state is given as $P = \frac{RT}{V - b}$ at $T$. Here,$b$ is the van der Waals constant. Which gas will exhibit a steeper increase in the plot of $Z$ (compression factor) versus $P$?

Under which of the following conditions does a real gas behave most like an ideal gas?

Under which conditions does a real gas show maximum deviation from ideal gas behavior?

$A$ $Van \ der \ Waals$ real gas acts as an ideal gas under which of the following conditions?